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Chemistry 1 > Topic 2- atomic structure and bonding > Flashcards

Topic 2- atomic structure and bonding Flashcards

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1
Q

Fill in table

Particle Relative mass Relative charge Location
Proton
Neutron
Electron

A

1, +1, nucleus
1, 0, nucleus
1/1840, -1, shell

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2
Q

What is an isotopes

A

Has the same number of protons but different number of neutrons therefore a different mass

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3
Q

What is the Relative atomic mass

A

The average mass e.g. For chlorine

(75x35)+(25x37)/ 100= 35.5

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4
Q

What is the plum pudding model
Label it
Who proposed the idea

A

The structure of an atom
It had a positive sphere ans negative electrons
J.J. Thompson

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5
Q

Groups go ______ and periods go _______ in the periodic table

A

Down and across

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6
Q

How many electron in group fives outer shell

A

Five

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7
Q

What is a positive ion called

What is a negative ion called

A

Cation

Anion

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8
Q

How is an ion formed

A

When an atom loses or gains an electron to gain a full outer shell

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9
Q

Simple negative ions change the end of their names to…

A

ide

Eg. Chloride

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10
Q

What is a molecular molecule

A

Contains more than one atom and are charged particles

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11
Q

What happens in a ionic bond

A

When there is a transfer of electrons to form a full outer shell
The attraction of oppositely charged ions

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12
Q

Ionic compounds do not have a _______ but the ions do have a _____

A

Charge

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13
Q 
What is the formula of 
sodium chloride 
Calcium chloride 
Magnesium oxide 
Potassium sulfite 
NOTE* group number/ valency will help
A

NaCl
CaCl2
MgO
K2S

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14
Q

What are subatomic particles?

A

Electrons, protons, neutrons

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15
Q

What are the properties of ionic compounds (6)

A

1) . High melting and boiling points
2) . Cannot conduct electricity when solid
3) . Can conduct electricity when liquid/ molten
4) . Lots of energy required to break down the forces of attraction
5) . Solid at room temperatures
6) . Most compounds can dissolve in liquids making them aqueous

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16
Q

Covalent bonding

A

Between two or more non-metals

Shared pair of electrons

17
Q

What is a diatomic molecule

A

They exist as molecules

Containing two atoms covalently bonded together

18
Q

Write the covalent bond of
Hydrogen
Chlorine
Oxygen

A

H-H
Cl-Cl
O=O

19
Q

What are the properties of simple covalent substance

A

Doesn’t conduct electricity
Usually gas or liquid at room temperature
Doesn’t electricity because no charged particles
Has weak forces of attraction, van dear Waals
Insoluble in water

20
Q

Give two examples of giant covalent substances

What element do they share in common?

A

Graphite and diamond

Carbon

21
Q

What is an allotrope

Give two examples

A

Different forms of the same element with the same physical state

22
Q

Give the properties of diamond

A

Carbon atom joined to four other carbon atoms
Tetrahedral
Has strong bonds between atoms, strong covalent atoms
Doesn’t conduct electricity because there are no free delocalised
electrons
High melting and boiling points
Insoluble in water

23
Q

What is diamond used for and give a reason

A

For cutting materials such as enamel (hardest substance in body) because diamond is the hardest substance on earth due it its tetrahedral shape

24
Q

Give the properties of graphite

A

Has strong covalent bonds between atoms
Has weak bonds between layers because of free delocalised electron
Joined to three other carbon atoms
Insoluble in water
Can conduct electricity
Cannot conduct electricity when molten/ liquid because structure is ruined
High melting and boiling points

25
Q

What is graphite used for

A

A lubricant because the weak force of attraction between the layers, due to a free delocalised electron, lets the layers slide over each other.

26
Q

Metallic bonding is caused by the _______ between _______ _______ and _______ ______ in the structure of the metal

A

Attraction
Delocalised electrons
Positive metal ions

27
Q

What is an alloy

A

Is a mixture of two or more elements which at least one is a metal eg. Brass

28
Q 
What is ... used for 
Aluminium 
Copper 
Iron 
Magnesium
A

Overhead power cables because of low density and good conductor of electricity
Electrical wires because of being a good conductor of electricity
For bridge and building because of high density and high melting and boiling points
For flares because it burns with a bright white light and also for strong alloys in aircraft because of low density

Chemistry 1 (8 decks)

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